Question

In a photosynthesis reaction 0.5796 grams of glucose was formed st a temp of 37.0 Celsius and 745 torr . How many milliliter did oxygen were formed with the glucose and how many were formed with the carbon dioxide . Vapor pressure is 50.0 torr

Answer 1

Balanced equation:
C₆H₁₂O₆ + 6 O₂ ===> 6 CO₂ + 6 H₂O
Reaction type: combustion

Moels of Glucose = 0.5796 /180.15 = 0.0032172 Moles

Moles of O2 needed =  0.01930 Moles

.Moles of CO2 formed =  0.01930 Moles

Volume of O2 and CO2 can be calculated using the formula

PV= nRT

P = Pressure in atm

V= Volume in Liter

n = no of moles

R = 0.0821 L atm K-1 Mol-1

T = Temperature in Kelvin

Volume of Oxygen

P = 745 - 50 = 0.9144 atm V= ? n =   0.01930 Moles T = 273 +37 = 310 K

V = nRT / P = 0.01930 x 0.0821 x 310 / 0.9144 = 0.5371 Liter or 537.1 ml

Volume of CO2

P = 745 - 50 = 0.9144 atm V= ? n =   0.01930 Moles T = 273 +37 = 310 K

V = nRT / P = 0.01930 x 0.0821 x 310 / 0.9144 = 0.5371 Liter or 537.1 ml

The volume of CO2 = 537.1 ml

The volume of O2 = 537.1 ml